Question

Draw the shapes of the following hybrid orbitals : (a) $sp_{2}$ (b) $sp_{3}$

Answer 1

Hybridization:

"Intermixing of atomic orbitals" with energy and shape in smaller difference; and redistribution of energies present in them to construct new orbitals of identical shape and equivalent energies.

Number of hybrid orbitals, $H\quad =\quad \frac { 1 }{ 2 } \left( { V }_{ e }\quad +\quad { N }_{ a }\quad +\quad { C }_{ a }\quad -\quad { C }_{ c } \right)$

Where,${ V }_{ e }$ = Number of valence electrons in the central atom.

${ N }_{ a }$ = Number of mono valent atoms joined to the central atom.

${ C }_{ a }$ = Magnitude of charge on anion.

${ C }_{ c }$ = Magnitude of charge on cation.

If value of H is 2 hybridization is sp.

If value of H is 3 hybridization is ${ sp }^{ 2 }$.

If value of H is 4 hybridization is ${ sp }^{ 3 }$.

Shape of ${ sp }^{ 2 }$ hybrid orbitals and shape of ${ sp }^{ 3 }$ hybrid orbitals are given below.